Which statement explains why covalent compounds generally have low melting points?
Weak intermolecular forces
In a covalent compound the atoms within a molecule are held together by strong shared pairs of electrons, but the separate molecules attract one another only through weak intermolecular forces.
Melting or boiling has to overcome those weak forces between molecules, not the strong bonds inside them, so relatively little energy is needed.
Covalent compounds have no free electrons and no metallic or strong ionic attractions, which is why they melt at far lower temperatures than ionic solids.
Hence, the answer is weak intermolecular forces.
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